Chemistry, 16.03.2020 21:05 chancecharles9oug353

Roasting galena [lead(II) sulfide] is an early step in the industrial isolation of lead. How many liters of sulfur dioxide, measured at STP, are produced by the reaction of 6.61 kg of galena with 154 L of oxygen gas at 220°C and 2.00 atm? Lead(II) oxide also forms.

Answers: 1

Show answers

Answers

Answer from: Shami7457

Answer : The volume of sulfur dioxide measured at STP is, 113.6 L

Explanation :

First we have to calculate the moles of PbS.

$\text{Moles of }PbS=\frac{\text{Mass of }PbS}{\text{Molar mass of }PbS}$

Molar mass of PbS = 239.27 g/mol

$\text{Moles of }PbS=\frac{6.61kg}{239.27g/mol}=\frac{6610g}{239.27g/mol}=27.62mol$

Now we have to calculate the moles of oxygen gas.

Using ideal gas equation:

PV=nRT

where,

P = Pressure of O_2 gas = 2.00 atm

V = Volume of O_2 gas = 154 L

n = number of moles O_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of O_2 gas = 220^oC=273+220=493K

Putting values in above equation, we get:

$2.00atm\times 154L=n\times (0.0821L.atm/mol.K)\times 493K$

n=7.61mol

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction will be:

$2PbS(s)+3O_2(g)\rightarrow 2PbO(s)+2SO_2(g)$

From the balanced chemical reaction we conclude that,

As, 3 moles of O_2 react with 2 moles of PbS

So, 7.61 moles of O_2 react with $\frac{2}{3}\times 7.61=5.07$ moles of PbS

From this we conclude that, PbS is an excess reagent because the given moles are greater than the required moles and O_2 is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of SO_2

From the reaction, we conclude that

As, 3 mole of O_2 react to give 2 mole of SO_2

So, 7.61 mole of O_2 react to give $\frac{2}{3}\times 7.61=5.07$ mole of SO_2

Now we have to calculate the volume of SO_2 at STP.

Using ideal gas equation:

PV=nRT

where,

P = Pressure of SO_2 gas = 1.00 atm

V = Volume of SO_2 gas = ?

n = number of moles SO_2 = 5.07 mol

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of SO_2 gas = 273 K

Putting values in above equation, we get:

$1.00atm\times V=5.07mol\times (0.0821L.atm/mol.K)\times 273K$

V=113.6L

Thus, the volume of sulfur dioxide measured at STP is, 113.6 L

Answer from: Quest

The answer is 3,5g co

Answer from: Quest

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

Another question on Chemistry

Chemistry, 22.06.2019 00:00

Alarge marble is dropped in a graduated cylinder with 35ml of water in it.the water level increases to 49ml.what is the volume of the marble

Answers: 1

Answer

Chemistry, 22.06.2019 08:30

Sally is making a model of a magnesium atom with an atomic mass number of 24 for her chemistry class. she has foam balls for the protons, neutrons, and electrons. she has added 6 neutrons to her model so far. how many more neutrons does she need to add to complete her neutral atom of magnesium?

Answers: 1

Answer

Chemistry, 22.06.2019 09:20

What happened to the amount of carbon dioxide in the atmosphere from 2010–2017?

Answers: 1

Answer

Chemistry, 22.06.2019 10:00

Drug abuse will not lead to physical and psychological dependence. true or false ?

Answers: 2

Answer

You know the right answer?

Roasting galena [lead(II) sulfide] is an early step in the industrial isolation of lead. How many li...